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How many grams of phosphorus react with 37.8 L of O2 at STP to form tetraphosphorus...
How many grams of phosphine (PH3) can form when 34.4 g of phosphorus and 87.7 L of hydrogen gas react at STP? P4(s) + H2(g) → PH3(g) (Unbalanced)
How many grams of phosphine (PH3) can form when 35.0 g of phosphorus and 96.2 L of hydrogen gas react at STP? P4(s) + H2(g) → PH3(g) (Unbalanced) ....... g PH3
1. How many ATOMS of phosphorus, are present in 4.10 moles of tetraphosphorus decaoxide, P4O10? __________ atoms of phosphorus 2. How many MOLES of oxygen are present in 1.75×1021 molecules of tetraphosphorus decaoxide? ___________ moles of oxygen 3. How many ATOMS of phosphorus are present in 7.95 grams of tetraphosphorus decaoxide, P4O10? ________atoms of phosphorus 4.How many GRAMS of oxygen are present in 1.75×1021 molecules of tetraphosphorus decaoxide? _________grams of oxygen
How many grams of phosphine (PH3) can form when 47.7 g of phosphorus and 95.2 L of hydrogen gas react at STP? P S)+H2(g)PH,) (Unbalanced) g PH
The elements phosphorus and oxygen react to give tetraphosphorus pentoxide according to the balanced equation: P4 +5O2 → P4O10 Suppose you have 0.5203 mol P4. (a) How many moles of O2 are needed for complete reaction? (b) What mass of P4O10, in grams, can be produced? (The molar mass of P4O10 is 283.88
. Tetraphosphorus decaoxide (P4010) reacts with H2O to form H2PO4. The balanced equation for this reaction is shown in Equation 11. P4010(s) + 6H2O(l) + 4H3PO4(4) (Eq. 11) Calculate the mass of H3PO4 that could possibly be produced by the reaction of 300 g of P4010 with 100 g of H2O. ning conner(IT)
How many grams of phosphorus (P4) are needed to completely consume 20.3 L of chlorine gas according to the following reaction at 25 °C and 1 atm? phosphorus (P4) ( s ) + chlorine ( g ) phosphorus trichloride ( l ) _____ grams phosphorus (P4)
How many grams of magnesium oxide form when 14.8 L of oxygen gas, measured at STP, completely reacts with magnesium metal according to this reaction? 2 Mg(s) + O2(g) → 2 MgO(s)
Phosphorus and liquid bromine react vigorously together to form phosphorus tribromide. P4 +6Br24 PBrz If 5.Og of phosphorus and 35g of bromine react, how many grams of PBr3 could be produced? Oa) 5 g PBrz Ob) 39.5 g PBr3 Oc) 79 g PBr3 Od) 0.146 g PBr3
1. How many grams of phosphorus (P4) are needed to completely consume 9.19 L of chlorine gas according to the following reaction at 25 °C and 1 atm? phosphorus (P4) ( s ) + chlorine ( g ) --->phosphorus trichloride ( l ) ____ grams phosphorus (P4) 2- What volume of oxygen gas is produced when 26.1 g of mercury(II) oxide reacts completely according to the following reaction at 25 °C and 1 atm? mercury(II) oxide (s) ---> mercury (l)...